btw.
5 grams of copper II sulfate was used
when it became an anyhride it had a mass of 0.15g

Are you sure you got that right? I assume that "it had a mass of..." means that the anhydride had a mass of... Is that right?

i know i made a mistake somewhere in my lab and i was wondering if you tell where my mistake is and what i should do. i would highly appreciate it.

so i know...
CuSO4 . 5H2O
molar weight is 249.69g

by itself is
CuSO4 = 159.61g
5H2O= 90.81

Good so far...

so i took the
mass of the water/total mass of hydrate x100= 36% of H2O removed in anhydrous copper (II) sulfate.

am i correct?
this is where i got confused...
-determine the # of moles of water present in each mole of hydrous copper (II) sulfate.

Here is where you strayed off course. The formula for your unknown hydrate is CuSO4 . XH2O. You need to solve for 'X', not assume that it is 5 and do some math without using any of the data you collected.